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Chemistry 122- Equilibrium Notes from Oct 11- Oct 13

by: Samantha Kessler

Chemistry 122- Equilibrium Notes from Oct 11- Oct 13 Chem 122

Marketplace > Truckee Meadows Community College > Chemistry > Chem 122 > Chemistry 122 Equilibrium Notes from Oct 11 Oct 13
Samantha Kessler


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About this Document

These notes cover equilibrium, Le Chatelier's principals, 5% rule, reaction quotient.
Chemistry 122
Kathleen Kolbet
Class Notes
General Chemistry, Equilibrium, LeChatelier's Principle
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This 3 page Class Notes was uploaded by Samantha Kessler on Monday October 17, 2016. The Class Notes belongs to Chem 122 at Truckee Meadows Community College taught by Kathleen Kolbet in Fall 2016. Since its upload, it has received 3 views. For similar materials see Chemistry 122 in Chemistry at Truckee Meadows Community College.


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Date Created: 10/17/16
Equilibrium Notes­ October 11, 2016 *Reactions at the forward rate and reverse rate have the same rate!* At equilibrium the rate=0 although the reaction rate has not stopped.   Reactants <­­­­­­­­­> Products  ­concentration stays constant  Kinetics­­­­­­> rate constant k  ­can not be written from the balanced equation  ­Temp effects ­Collisions  ­Ea  ­need to know units Equilibrium ­­­­­> equilibrium constant K ­T dependent  ­can be written from a balanced equation  ­can be treated like an elementary steps in mechanism.  ­No units!!!  Ex. Forward direction: HC 2H3O2(aq)­­­­­­> H+(aq)+C2H3O 2­ (aq)            rate= kf=[HC3H3O2] Reverse direction  H+ (aq)+ C2H3O2(aq)­­­­­­>HC2H3O2(aq) rate= kr=[H+][C2H3O2­] *These are going just as fast forward as it is fast.* kf=[HC2H3O2]=kr[H+][C2H3O2­]    kf          [H+][C2H3O2­]            Products ­­­­­­­  = ­­­­­­­­­­­­­­­­­­­­­­­­  =    ­­­­­­­­­­­­­­­­­­    kr            [HC2H3O2]                Reactants *Ignore solids and liquids because their  consent stays the same. (Kc=concentrations or K) (Kp=pressures for gasses)  *When K>1,000, then there are more products than reactants. Reaction then favors the  products.  *When K < (1/1000) then there are more reactants than products. Reactions favor reactants.  REVIST ACIDS,BASES,STONG & WEAK ACIDS  ­Changes in pressure for gasses its like changing concentration.  ­Increase volume/decrease pressure. # of particles (g) = (total pressure/total volume)  Le Chatelier’s Principal Heat+ R <­­­­­> P                                             Endothermic­­­­­>  △H>0 Increase T-----> shift forward ------> K increases R---->P+heat exothermic △H<0 Increase T----> shift reverse ---->K decreases Decrease T----> shift forward ----> K increases positive catalysis= speeds up reaction /lowers activation energy rate (does not change the ration. gets to equilibrium faster) negative catalysis= slows down reaction/raises the activation energy. October 13,2016 Kp=Kc(RT)△n Ni(CO)4 (g) <----> Ni(s) + 4CO(g), Kp=0.0047 See examples in workbook Q= reaction quotient =same expression as K (equilibrium) but we are not at equilibrium ex: PCO4 Kp=------- ( at equilibrium) PNi(CO)4 PCO4 Q= --------- (not at equilibrium) PNi(CO)4 Q>K-----> reverses shift Q<K----->forward shift Q=K----->at equilibrium Alternatives for roots in the calculator √ ­­­­­­> ^(1/2)  3rd √­­­­­>(1/3)  5% rule: if K<1X10­3 , then the shift forward is very small...less than 5% of the initial  concentration. We ignore when x is being added or subtracted in K 


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